Solubility Product Problems (15-17

PAGE NO. # 1
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DPP No.# 55
Solubility product
1. Write the equation for dissociation of following salts and determine their solubility in terms of Ksp
.
(i) PbBr2
(ii) Hg2
CrO4
(iii) BaC2
O4
(iv) Fe(OH)3
(v)Ag2
CO3
(vi) Sb2
S3
(vii)AgCNS (viii)Ag3
PO4
(ix) Li3
Na3
(AlF6
)2
(x) Hg2
I2
(xi) Ba3
(PO4
)2
(xii) Ca5
(PO4
)3
F
(xiii) A3
B4
(xiv) CaF2
(xv)Ag2
CrO4
2. (i) Ksp
of AgCl is 1.8 × 10–10
. The solubility of AgCl in pure water in moles/litre :
(A) 1.34 × 10–5
(B) 4.24 × 10–5
(C) 1.8 × 10–5
(D) 3.6 × 10–5
(ii) In the above question the solubility in gram per litre will be –
(A) 180.26 × 10–5
(B) 192.29 × 10–5
(C) 210 × 10–4
(D) 176.85 × 10–4
3. Calculate solubility of AB2
in pure water. Ksp
of AB2
= 25.6 × 10–8,
4. Solubility of a A2
B salt in pure water is 2 × 10–5
moles in 100 ml. Calculate Ksp
of salt.
5. Ksp
of AgBr is 4 × 10–13
and [Al+
] is a solution is 1 × 10–6
m/l what is [Br–
] in that solution.
6. If Ksp
of AgI is 8.5 × 10–17
. The maximum amount of AgI which can be dissolved in 2500 ml of water will be –
(A) 9.22 × 10–9
gm (B) 2.3 × 108
gm (C) 5.42 × 10–5
gm (D) 2.17 × 10–5
gm
7. The volume of water needed to dissolve 1 g of BaSO4
(Ksp
= 1.1 × 10–10
) at 25ºC is –
(A) 820 litre (B) 410 litre (C) 205 litre (D) none of these
8. How many grams of CaC2
O4
will dissolve in distilled water to make one litre of saturated solution of it ?
(Ksp
of CaC2
O4
= 2.5 × 10–9
mol2
lit–2
)
(A) 0.0064 gm (B) 0.1028 gm (C) 0.1280gm (D) 0.2056 gm
9. At 20ºC, the Ag+
ion concentration in a saturated solution Ag2
CrO4
is 1.5 × 10–4
mole/lit. At 20ºC, the
solubility product of Ag2
CrO4
could be –
(A) 3.37 × 10–12
(B) 1.68 × 10–10
(C) 1.68 × 10–12
(D) 1.12 × 10–10
10. In the system CaF2
(s) Ca2+
(ag) + 2F–
increasing the concentration of Ca2+
ions 4 times will cause the eq. concentration of F–
ions to change to
.............. times the initial value.
(A) 4 (B) 1/2 (C) 2 (D) 1/4
11. Concentration ofAg+
ion in a saturated solution ofAg2
CrO4
is 5.4 × 10–6
g/litre when the salt is 50% dissociated.
Then solubility product of Ag2
CrO4
is –
(A) 7.03 × 10–17
(B) 6.25 × 10–23
(C) 1.72 × 10–23
(D) 2.15 × 10–24
12. (i) For an experiment Pb(OH)2
is taken , if salt is 80% dissociated & Ksp
of Pb(OH)2
is 8 × 10–6
. Then solubility
of salt in moles/litre is –
(A) 1.57 × 10–2
(B) 2 × 10–2
(C) 1.26 × 10–5
(D) 2.3 × 10–2
(ii) Considering the above question, what will be the solubility in gms/litre –
(A) 3.32 (B) 3.65 (C) 3.05 (D) 3.79
PHYSICALINORGANIC
CHEMISTRY
DAILY PRACTICE PROBLEMS
D P P
COURSE NAME : UMANG (UP) DATE : 23.09.2013 to 28.09.2013 DPP NO. 55 & 57
TARGET
JEE (ADVANCED) : 2014

PAGE NO. # 2
13. pH of a saturated solution of A(OH)3
is 10. Calculate Ksp
of A(OH)3
at 25ºC.
14. Solubility of As2
S3
is 7.38 mg in 10ml of water. Calculate Ksp
of As2
S3
.
15. Ksp
of A3
B4
is 6.912 × 10–18
. Calculate solubility of A3
B4
.
DPP No.# 56
1.(a) The solubility of A2
X is y mol dm 3
. Its solubility product is :
(A) 6 y4
(B) 64 y4
(C) 36 y5
(D) 4 y3
(b) The solubility of sparingly soluble electrolyte Mm
Aa
in water is given by the expression :
(A) s =
am
am
sp
am
K









(B) s =
am/1
am
sp
am
K









(C) s =
am
ma
sp
am
K









(D) s =
am/1
ma
sp
am
K









2.(a) Three sparingly soluble salts M2
X, MX and MX3
have the solubility product are in the ratio of 4: 1 : 27. Their
solubilities will be in the order
(A) MX3
> MX > M2
X (B) MX3
> M2
X > MX (C) MX > MX3
> M2
X (D) MX > M2
X > MX3
(b) A particular saturated solution of silver chromate, Ag2
CrO4
, has [Ag+
]= 5×10–5
and [CrO4
2–
] = 4.4×10–4
M.
What is value of Ksp
forAg2
CrO4
?
(A) 1.1 × 10–12
. (B) 1.5 × 10–12
(C) 2 × 10–6
(D) 1 × 1012
.
3.(a) If the solubility product of silver oxalate is 5 × 10–10
, what will be the weight of Ag2
C2
O4
in 2.5 litres of a
saturated solution ? (Ag = 108, C = 12, O = 16).
(A) 0.50 gm (B) 0.38 gm (C) 0.30 gm (D) 0.45 gm.
(b) A student wants to prepare a saturated solution of Ag+
ion . He has got three samples AgCl (Ksp
= 10 10
),
AgBr (Ksp
= 1.6 × 1013
) and Ag2
CrO4
(Ksp
= 3.2 × 1011
) . Which of the above compound will be used by him
using minimum weight to prepare 1 lit. of saturated solution.
(A)AgCl (B)AgBr (C)Ag2
CrO4
(D) all the above .
4.(a) If the solubility of Ag2
SO4
in 10–2
M Na2
SO4
solution be 2 × 10–8
M then Ksp
of Ag2
SO4
will be:
(A) 32 × 10–24
(B) 16 × 10–18
(C) 32 × 10–18
(D) 16 × 10–24
(b) The solubility of CaF2
in water at 1518ºC is 2 × 10–4
mole/litre. Calculate Ksp
of CaF2
and its solubility in 0.1M
NaF solution.
(A) 3.5 × 108
mole/litre (B) 3.0 × 109
mole/litre. (C) 3.3 × 10–9
mole/litre (D) 4.0 × 107
mole/litre
5.(a) Calculate F—
in a solution saturated with respect of both MgF2
and SrF2
.
Ksp
(MgF2
) = 9.5 x 10-9
, Ksp
(SrF2
) = 4 x 10-9
.
(A) 3 × 10–3
M. (B) 4 × 10–2
M. (C) 3.5 × 10–3
M (D) 1 × 10–3
M.
(b) A solution is saturated with respect to SrCO3
& SrF2
. The [CO3
2
] was found to be 1.2 x 103
M. The
concentration of F
in the solution would be : Ksp
(SrCO3
) = 10–9
, Ksp
(SrF2
) = 3 × 10–11
.
(A) 3 x 103
M (B) 2 x 102
M (C) 6 x 102
M (D) 6 x 107
M
6. Calculate the solubility of AgCl (s) in
(a) pure water (b) 0.1 M NaCl (c) 0.01 M CaCl2
at 25º C .
Ksp
(AgCl) = 2.56  1010
.Comment on the influence of [Cl
] on the solubility of AgCl.
7. Find the solubility of CaF2
in 0.5 M solution of CaCl2
and water. How many times in solubility in the second
case greater than in the first ? Ksp
(CaF2
) = 3.2 × 10–11
.
8. If you place the amounts given below in pure water, will all of the salt dissolve before equilibrium can be
established, or will some salt remain undissolved ?
(a) 4.96 mg of MgF2
in 125 ml of pure water, Ksp
= 3.2 x 10-8
(b) 3.9 mg of CaF2
in 100 ml of pure water, Ksp
= 4 x 10-12
Also find the percentage saturation in each case.

PAGE NO. # 3
DPP No.# 57
Solubility in presence of common ion
1. Solubility product of AgCl is 1.8 × 10–10
, then find out solubility of AgCl in
(i) 0.1M NaCl
(A) 3.6 × 10–10
(B) 1.8 × 10–10
(C) 3.6 × 10–9
(D) 1.8 × 10–9
(ii) 0.2MAgNO3
(A) 3 × 10–10
(B) 0.36 × 10–10
(C) 9 × 10–10
(D) 2.6 × 10–10
(iii) 2M CaCl2
(A) 9 × 10–10
(B) 4.5 × 10–11
(C) 1.5 × 10–11
(D) 6 × 10–11
(iv) (iv) pure water.
(A) 1.34 × 10–5
(B) 4.34 × 10–5
(C) 2.87 × 10–5
(D) 1.89 × 10–5
2. Ksp
of PbCl2
is 4 ×10–15
calculate its solubility in :
(i) pure water
(ii) 0.2 M AlCl3
solution
(iii) 5 × 10–3
M Pb3
(PO4
)2
solution
(iv) 0.02 M NaCl solution
(v) 0.4 M Pb(NO3
)2
solution
3. The solubility of AgCl will be minimum in –
(A) 0.01 M AgNO3
(B) pure water (C) 0.01 M CaCl2
(D) 0.1 M NaCl
4. The solubility product of AgCl is 4 × 10–10
at 298 K. The solubility of AgCl in 0.04 M CaCl2
will be–
(A) 2 × 10–5
M (B) 1 × 10–4
M (C) 5 × 10–9
M (D) 2.2 × 10–4
M
5. The molar solubility of PbI2
in 0.2 M Pb(NO3
)2
solution in terms of solubility product, Ksp
of PbI2
is–
(A)
2/1
sp
2.0
K








(B)
2/1
sp
8.0
K








(C)
3/1
sp
8.0
K








(D)
2/1
sp
4.0
K








6. Ksp
of Zn(OH)2
is 4.5 × 10–17
then its solubility in a solution having pH = 10 will be –
(A) 4.5 × 10–10
(B) 1.4 × 10–10
(C) 6.7 × 10–10
(D) 7.6 × 10–10
7. Solubility of Mg(OH)2
having Ksp
equal to 8.9 × 10–13
, in a solution containing 500 ml of 0.2 M NH4
OH and 500
ml of 0.4 M Ca(OH)2
is –
(A) 3.4 × 10–19
(B) 55.63 × 10–13
(C) 2.34 × 10–9
(D) 8.34 × 10–13
8. Molar solubility of As2
S3
in 0.3 M Al2
S3
solution in terms of solubility product Ksp
of As2
S3
is–
(A)
918.2
Ksp
(B)
916.2
K
3
sp
(C)
2.1
Ksp
(D)
2.1
K
3
sp
9. Ksp
of PbI2
is 8 × 10–12
. A solution contains 2 × 10–3
M Pb+2
ions and 2 × 10–4
M I–
ions. Predict ppt of PbI2
will
form or not.
11. The precipitate of CaF2
(Ksp
= 1.7 × 10–10
) is obtained when equal volumes of the following are mixed–
(A) 10–4
Ca2+
+ 10–4
M F–
(B) 10–2
M Ca2+
+ 10–3
M F–
(C) 10–5
M Ca2+
+ 10–3
M F–
(D) 10–3
M Ca2+
and 10–3
M F–

PAGE NO. # 4
12. To Ag2
CrO4
solution over its own precipitate, CrO4
–2
ions are added. This result in
(A) increase in Ag+
concentration (B) decrease in Ag+
concentration
(C) increase in solubility product (D) None of these
13. What is the minimum concentration of SO4
2–
required to precipitate BaSO4
in a solution containing
1 × 10–4
mole of Ba2+
? Ksp
for BaSO4
= 4 × 10–10
(A) 4 × 10–10
M (B) 4 × 10–6
M (C) 2 × 10–7
M (D) 2 × 10–3
M
14. What would be the pH at which Fe(OH)2
begins to precipitate from a solution containing 0.009 M Fe+2
ions.
Ksp
of Fe(OH)2
is 1.8 × 10–15
.
(A) 8.37 (B) 6.35 (C) 7.65 (D) 9.28
15. How many grams of CaBr2
(MM = 200) can be added to 250 ml of 0.01 M solution of silver nitrate to just start
the precipitation of silver bromide. Ksp
of AgBr is 5.0 × 10–13
.
16. A solution contains 0.1 M Zn+2
ions and is saturated with H2
S. Calculatee amount of HCl which should be
added in 500 ml of solution to prercipitate ZnS. Ksp
of ZnS = 13.5 × 10–23
. K1
of H2
S = 10–7
and K2
of
H2
S = 1.5 × 10–14
concentration of H2
S in saturated solutin is 0.1N.
17. A solution has 0.02 M A+2
and 0.1M NH4
OH calculate the concentration of NH4
Cl required to prevent the
formation of A(OH)2
in solution. Ksp
of A(OH)2
is 2 × 10–12
and Kb
of NH4
OH is 10–5
.
ANSWER KEY
DPP No.# 55
2. (i) (A) (ii) (B) 3. Ksp
of AB2
= 25.6 × 10–8,
A = 4 × 10–3
m/l 4. 3.2 ×10–11
5. Br–
= 4 × 10–7
m/l 6. (C) 7. (B) 8. (A) 9. (C)
10. (B) 11. (B) 12. (i) (A) (ii) (D) 13. 3.34 × 10–17
14. 26.24 × 10–12
15. 10–3
m/l
DPP No.# 56
1.(a) (D) (b) (B) 2.(a) (B) (b) (A) 3.(a) (B) (b) (B)
4.(a) (B) (b) (C) 5.(a) (A) (b) (C)
6. (a) 1.6 × 10 -5
mol/lit. (b) 2.56 × 10 -9
mol/lit. (c) 1.28 × 10–8
mol/lit.
7. 4 × 10–6
M, 2 × 10–4
M, 50 times.
8. (a) Will dissolve, 32% saturation (b) will not dissolve, 100% saturation.
DPP No.# 57
Solubility in presence of common ion
1. (i) (D) 1.8 × 10–9
(ii) (C) (iii) (B) (iv) (A)
2. (i)10–5
M (ii) 1.11 × 10–14
M (iii) 2.58 ×10–7
M (iv) 10–11
M (v) 5 × 10–8
M
3. (C) 4. (C) 5. (B) 6. (A) 7. (B) 8. (A) 9. Yes
11. (B) 12. (B) 13. (B) 14. (C) 15. 1.25 × 10–9
gm 16. 6.01 gm
17. 0.1 M

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